Please Wait... While Loading Full Video### Conductance of Electrolytic Solutions and Kohlrausch Law

● Conductance of Electrolytic Solutions

● Measurement of the Conductivity of Ionic Solutions

● Variation of Conductivity and Molar Conductivity with Concentration

`=>` For Strong Electrolytes

`=>` For Weak Electrolytes

● Kohlrausch Law of Independent Migration of Ions

● Applications of Kohlrausch Law

● Measurement of the Conductivity of Ionic Solutions

● Variation of Conductivity and Molar Conductivity with Concentration

`=>` For Strong Electrolytes

`=>` For Weak Electrolytes

● Kohlrausch Law of Independent Migration of Ions

● Applications of Kohlrausch Law

First, we will define a few terms before we consider the subject of conductance of electricity through electrolytic solutions.

`color{green}("Resistance") :` The electrical resistance is represented by the symbol `‘R’` and it is measured in ohm `(Ω)` which in terms of `SI` base units is equal to `color{red}((kg m^2)/(s^3 A^2))`. It can be measured with the help of a Wheatstone bridge. The electrical resistance of any object is directly proportional to its length, `l`, and inversely proportional to its area of cross section, `A`. That is,

`color{red}(R prop l/A)` or `color{red}(R = rho l/A)` ............(1)

`color{green}("Resistivity") :` The constant of proportionality, `ρ` (Greek, rho), is called resistivity (specific resistance).

`=>` Its `SI` units are ohm metre `(Ω m)` and quite often its submultiple, ohm centimetre `(Ω cm)` is also used.

`=>` IUPAC recommends the use of the term resistivity over specific resistance.

`=>` The resistivity for a substance is its resistance when it is one metre long and its area of cross section is one `m^2`.

It can be seen that :

`color{red}(1 Ω m = 100 Ω cm & 1 Ω cm = 0.01 Ω m)`

`color{green}("Conductance") :` The inverse of resistance, `R`, is called conductance, `G`, and we have the relation :

`color{red}(G = 1/R = A/(rho l) = k A/l)` ..............(2).

`=>` The SI unit of conductance is siemens, represented by the symbol `‘S’` and is equal to `ohm^(–1)` (also known as mho) or `Ω^(–1)`.

`color{green}text(Conductivity) :` The inverse of resistivity, called conductivity (specific conductance) is represented by the symbol, `κ` (Greek, kappa).

`=>` IUPAC has recommended the use of term conductivity over specific conductance.

`=>` The SI units of conductivity are `S m^(–1)` but quite often, `κ` is expressed in `S cm^(–1)`.

`=>` Conductivity of a material in `S m^(–1)` is its conductance when it is `1 m` long and its area of cross section is `1 m^2`.

`=>` `color{red}(1 S cm^(–1) = 100 S m^(–1))`.

`=>` It can be seen from Table that the magnitude of conductivity varies a great deal and depends on the nature of the material.

`=>` It also depends on the temperature and pressure at which the measurements are made.

`=>` Materials are classified into conductors, insulators and semiconductors depending on the magnitude of their conductivity.

`=>` Metals and their alloys have very large conductivity and are known as conductors. Certain non-metals like carbon-black, graphite and some organic polymers* are also electronically conducting.

`=>` Substances like glass, ceramics, etc., having very low conductivity are known as insulators.

`=>` Substances like silicon, doped silicon and gallium arsenide having conductivity between conductors and insulators are called semiconductors and are important electronic materials.

`=>` Certain materials called superconductors by definition have zero resistivity or infinite conductivity.

`=>` Earlier, only metals and their alloys at very low temperatures (`0` to `15 K`) were known to behave as superconductors, but nowadays a number of ceramic materials and mixed oxides are also known to show superconductivity at temperatures as high as `150 K`.

`color{green}text(Electrical Conductance) :` Electrical conductance through metals is called metallic or electronic conductance and is due to the movement of electrons.

`=>` The electronic conductance depends on

(i) the nature and structure of the metal

(ii) the number of valence electrons per atom

(iii) temperature (it decreases with increase of temperature).

`=>` As the electrons enter at one end and go out through the other end, the composition of the metallic conductor remains unchanged. The mechanism of conductance through semiconductors is more complex.

We know that even very pure water has small amounts of hydrogen and hydroxyl ions `(~10^(–7M))` which give it very low conductivity `(3.5 × 10^(–5) S m^(–1))`. When electrolytes are dissolved in water, they furnish their own ions in the solution hence its conductivity also increases.

`color{green}("Ionic Conductivity") :` The conductance of electricity by ions present in the solutions is called electrolytic or ionic conductance.

`=>` The conductivity of electrolytic (ionic) solutions depends on :

(i) the nature of the electrolyte added

(ii) size of the ions produced and their solvation

(iii) the nature of the solvent and its viscosity

(iv) concentration of the electrolyte

(v) temperature (it increases with the increase of temperature).

Passage of direct current through ionic solution over a prolonged period can lead to change in its composition due to electrochemical reactions.

`color{green}("Resistance") :` The electrical resistance is represented by the symbol `‘R’` and it is measured in ohm `(Ω)` which in terms of `SI` base units is equal to `color{red}((kg m^2)/(s^3 A^2))`. It can be measured with the help of a Wheatstone bridge. The electrical resistance of any object is directly proportional to its length, `l`, and inversely proportional to its area of cross section, `A`. That is,

`color{red}(R prop l/A)` or `color{red}(R = rho l/A)` ............(1)

`color{green}("Resistivity") :` The constant of proportionality, `ρ` (Greek, rho), is called resistivity (specific resistance).

`=>` Its `SI` units are ohm metre `(Ω m)` and quite often its submultiple, ohm centimetre `(Ω cm)` is also used.

`=>` IUPAC recommends the use of the term resistivity over specific resistance.

`=>` The resistivity for a substance is its resistance when it is one metre long and its area of cross section is one `m^2`.

It can be seen that :

`color{red}(1 Ω m = 100 Ω cm & 1 Ω cm = 0.01 Ω m)`

`color{green}("Conductance") :` The inverse of resistance, `R`, is called conductance, `G`, and we have the relation :

`color{red}(G = 1/R = A/(rho l) = k A/l)` ..............(2).

`=>` The SI unit of conductance is siemens, represented by the symbol `‘S’` and is equal to `ohm^(–1)` (also known as mho) or `Ω^(–1)`.

`color{green}text(Conductivity) :` The inverse of resistivity, called conductivity (specific conductance) is represented by the symbol, `κ` (Greek, kappa).

`=>` IUPAC has recommended the use of term conductivity over specific conductance.

`=>` The SI units of conductivity are `S m^(–1)` but quite often, `κ` is expressed in `S cm^(–1)`.

`=>` Conductivity of a material in `S m^(–1)` is its conductance when it is `1 m` long and its area of cross section is `1 m^2`.

`=>` `color{red}(1 S cm^(–1) = 100 S m^(–1))`.

`=>` It can be seen from Table that the magnitude of conductivity varies a great deal and depends on the nature of the material.

`=>` It also depends on the temperature and pressure at which the measurements are made.

`=>` Materials are classified into conductors, insulators and semiconductors depending on the magnitude of their conductivity.

`=>` Metals and their alloys have very large conductivity and are known as conductors. Certain non-metals like carbon-black, graphite and some organic polymers* are also electronically conducting.

`=>` Substances like glass, ceramics, etc., having very low conductivity are known as insulators.

`=>` Substances like silicon, doped silicon and gallium arsenide having conductivity between conductors and insulators are called semiconductors and are important electronic materials.

`=>` Certain materials called superconductors by definition have zero resistivity or infinite conductivity.

`=>` Earlier, only metals and their alloys at very low temperatures (`0` to `15 K`) were known to behave as superconductors, but nowadays a number of ceramic materials and mixed oxides are also known to show superconductivity at temperatures as high as `150 K`.

`color{green}text(Electrical Conductance) :` Electrical conductance through metals is called metallic or electronic conductance and is due to the movement of electrons.

`=>` The electronic conductance depends on

(i) the nature and structure of the metal

(ii) the number of valence electrons per atom

(iii) temperature (it decreases with increase of temperature).

`=>` As the electrons enter at one end and go out through the other end, the composition of the metallic conductor remains unchanged. The mechanism of conductance through semiconductors is more complex.

We know that even very pure water has small amounts of hydrogen and hydroxyl ions `(~10^(–7M))` which give it very low conductivity `(3.5 × 10^(–5) S m^(–1))`. When electrolytes are dissolved in water, they furnish their own ions in the solution hence its conductivity also increases.

`color{green}("Ionic Conductivity") :` The conductance of electricity by ions present in the solutions is called electrolytic or ionic conductance.

`=>` The conductivity of electrolytic (ionic) solutions depends on :

(i) the nature of the electrolyte added

(ii) size of the ions produced and their solvation

(iii) the nature of the solvent and its viscosity

(iv) concentration of the electrolyte

(v) temperature (it increases with the increase of temperature).

Passage of direct current through ionic solution over a prolonged period can lead to change in its composition due to electrochemical reactions.

Measurement of an unknown resistance can be performed on a Wheatstone bridge. For measuring the resistance of an ionic solution we face two problems.

(i) Passing direct current (DC) changes the composition of the solution.

(ii) A solution cannot be connected to the bridge like a metallic wire or other solid conductor.

`=>` The first difficulty is resolved by using an alternating current (AC) source of power.

`=>` The second problem is solved by using a specially designed vessel called conductivity cell.

`color{green}("Conductivity Cell") :` It is available in several designs and two simple ones are shown in Fig

`=>` Basically it consists of two platinum electrodes coated with platinum black (finely divided metallic `Pt` is deposited on the electrodes electrochemically).

`=>` These have area of cross section equal to `‘A’` and are separated by distance `‘l’.` Therefore, solution confined between these electrodes is a column of length `l` and area of cross section A.

`=>` The resistance of such a column of solution is then given by the equation :

`color{red}(R = ρ l/A = l/(k A))`

`=>` The quantity `l/A` is called cell constant denoted by the symbol, `G^**`.

`=>` It depends on the distance between the electrodes and their area of cross-section and has the dimension of length`text()^(–1)` and can be calculated if we know `l` and `A`.

`=>` Measurement of `l` and `A` is not only inconvenient but also unreliable.

`color{green}("Measurement of Cell Constant") :`

`=>` The cell constant is usually determined by measuring the resistance of the cell containing a solution whose conductivity is already known. For this purpose, we generally use `KCl` solutions whose conductivity is known accurately at various concentrations (Table) and at different temperatures.

`=>` The cell constant, `G^**`, is then given by the equation :

`color{red}(G^(**) = l/A = R k)` ............(3)

`=>` Once the cell constant is determined, we can use it for measuring the resistance or conductivity of any solution. The set up for the measurement of the resistance is shown in Fig

`=>` It consists of two resistances `R_3` and `R_4`, a variable resistance `R_1` and the conductivity cell having the unknown resistance `R_2`.

`=>` The Wheatstone bridge is fed by an oscillator `O` (a source of a.c. power in the audio frequency range `550` to `5000` cycles per second). `P` is a suitable detector (a headphone or other electronic device) and the bridge is balanced when no current passes through the detector. Under these conditions :

Unknown resistance `color{red}(R_2 = (R_1 R_4)/R_3)` .................(4)

`=>` Now a days, inexpensive conductivity meters are available which can directly read the conductance or resistance of the solution in the conductivity cell.

`=>` Once the cell constant and the resistance of the solution in the cell is determined, the conductivity of the solution is given by the equation :

`color{red}(k = text(cell constant)/R = (G^(**))/R)` ..............(5).

`=>` The conductivity of solutions of different electrolytes in the same solvent and at a given temperature differs due to charge and size of the ions in which they dissociate, the concentration of ions or ease with which the ions move under a potential gradient.

`=>` Therefore, it becomes necessary to define a physically more meaningful quantity called molar conductivity denoted by the symbol `Λ_m` (Greek, lambda).

`color{green}("Molar Conductivity") :` Molar conductivity is related to the conductivity of the solution by the equation :

Molar conductivity ` color{red}(= Λ_m = k/C)` ..................(6).

In the above equation, if `κ` is expressed in `S m^(–1)` and the concentration, `c` in `mol m^(-3)` then the units of `Λ_m` are in `Sm^2 mol^(-1)`. It may be noted that :

`color{red}(1 mol m^(-3) = 1000(L/m^3) xx text{molarity (mol/L)})`

Hence, `color{red}(Λ_m(S m^2 mol^(–1)) = (k (S m^(-1)))/(1000 L m^(-3) xx (text{molarity} (mol L^(-1))))`

If we use `S cm(-1)` as the units for `κ` and mol `cm^(-3)`, the units of concentration, then the units for `Λ_m` are `S cm^2 mol^(–1)`.

It can be calculated by using the equation :

`color{red}(Lambda_m (S cm^2 mol^(-1)) = (k (S cm^(-1) ) xx 1000 (cm^3//L))/text{molarity (mol/L)})`

Both type of units are used in literature and are related to each other by the equations :

`color{red}(1 S m^2mol^(–1) = 10^4 S cm^2mol^(–1)` or `1 S cm^2mol^(–1) =10–4 S m^2mol^(–1))`

(i) Passing direct current (DC) changes the composition of the solution.

(ii) A solution cannot be connected to the bridge like a metallic wire or other solid conductor.

`=>` The first difficulty is resolved by using an alternating current (AC) source of power.

`=>` The second problem is solved by using a specially designed vessel called conductivity cell.

`color{green}("Conductivity Cell") :` It is available in several designs and two simple ones are shown in Fig

`=>` Basically it consists of two platinum electrodes coated with platinum black (finely divided metallic `Pt` is deposited on the electrodes electrochemically).

`=>` These have area of cross section equal to `‘A’` and are separated by distance `‘l’.` Therefore, solution confined between these electrodes is a column of length `l` and area of cross section A.

`=>` The resistance of such a column of solution is then given by the equation :

`color{red}(R = ρ l/A = l/(k A))`

`=>` The quantity `l/A` is called cell constant denoted by the symbol, `G^**`.

`=>` It depends on the distance between the electrodes and their area of cross-section and has the dimension of length`text()^(–1)` and can be calculated if we know `l` and `A`.

`=>` Measurement of `l` and `A` is not only inconvenient but also unreliable.

`color{green}("Measurement of Cell Constant") :`

`=>` The cell constant is usually determined by measuring the resistance of the cell containing a solution whose conductivity is already known. For this purpose, we generally use `KCl` solutions whose conductivity is known accurately at various concentrations (Table) and at different temperatures.

`=>` The cell constant, `G^**`, is then given by the equation :

`color{red}(G^(**) = l/A = R k)` ............(3)

`=>` Once the cell constant is determined, we can use it for measuring the resistance or conductivity of any solution. The set up for the measurement of the resistance is shown in Fig

`=>` It consists of two resistances `R_3` and `R_4`, a variable resistance `R_1` and the conductivity cell having the unknown resistance `R_2`.

`=>` The Wheatstone bridge is fed by an oscillator `O` (a source of a.c. power in the audio frequency range `550` to `5000` cycles per second). `P` is a suitable detector (a headphone or other electronic device) and the bridge is balanced when no current passes through the detector. Under these conditions :

Unknown resistance `color{red}(R_2 = (R_1 R_4)/R_3)` .................(4)

`=>` Now a days, inexpensive conductivity meters are available which can directly read the conductance or resistance of the solution in the conductivity cell.

`=>` Once the cell constant and the resistance of the solution in the cell is determined, the conductivity of the solution is given by the equation :

`color{red}(k = text(cell constant)/R = (G^(**))/R)` ..............(5).

`=>` The conductivity of solutions of different electrolytes in the same solvent and at a given temperature differs due to charge and size of the ions in which they dissociate, the concentration of ions or ease with which the ions move under a potential gradient.

`=>` Therefore, it becomes necessary to define a physically more meaningful quantity called molar conductivity denoted by the symbol `Λ_m` (Greek, lambda).

`color{green}("Molar Conductivity") :` Molar conductivity is related to the conductivity of the solution by the equation :

Molar conductivity ` color{red}(= Λ_m = k/C)` ..................(6).

In the above equation, if `κ` is expressed in `S m^(–1)` and the concentration, `c` in `mol m^(-3)` then the units of `Λ_m` are in `Sm^2 mol^(-1)`. It may be noted that :

`color{red}(1 mol m^(-3) = 1000(L/m^3) xx text{molarity (mol/L)})`

Hence, `color{red}(Λ_m(S m^2 mol^(–1)) = (k (S m^(-1)))/(1000 L m^(-3) xx (text{molarity} (mol L^(-1))))`

If we use `S cm(-1)` as the units for `κ` and mol `cm^(-3)`, the units of concentration, then the units for `Λ_m` are `S cm^2 mol^(–1)`.

It can be calculated by using the equation :

`color{red}(Lambda_m (S cm^2 mol^(-1)) = (k (S cm^(-1) ) xx 1000 (cm^3//L))/text{molarity (mol/L)})`

Both type of units are used in literature and are related to each other by the equations :

`color{red}(1 S m^2mol^(–1) = 10^4 S cm^2mol^(–1)` or `1 S cm^2mol^(–1) =10–4 S m^2mol^(–1))`

Q 2927634581

Resistance of a conductivity cell filled with `0.1 mol L^(–1) KCl` solution is `100 Ω`. If the resistance of the same cell when filled with `0.02 mol L^(–1) KCl` solution is `520 Ω`, calculate the conductivity and molar conductivity of `0.02 mol L^(–1) KCl ` solution. The conductivity of `0.1 mol L^(–1) KCl` solution is `1.29 S//m`.

The cell constant is given by the equation:

Cell constant = G* = conductivity × resistance

`= 1.29 S//m × 100 Ω = 129 m^(–1) = 1.29 cm^(–1)`

Conductivity of `0.02 mol L^(–1) KCl` solution = cell constant / resistance

`G^(**)/R = (129 m^(-1))/(520 Omega) = 0.248 S m^(-1)`

Concentration ` = 0.02 mol L^(-1)`

` = 1000xx0.02 mol m^(-3)`

` = 20 mol m^(-3)`

Molar conductivity `=Λ_m = (kappa)/c`

` = (248xx10^(-3) S m^(-1))/(20 mol m^(-3))`

` = 124xx10^(-4) S m^2 mol^(-1)`

Alternatively, `κ = (1.29 cm^(-1))/(520 Omega)`

` = 0.248 xx 10^(-2) S cm^(-1)` and `Λ_m = kappa x 1000 cm^3 L^(-1) ` molarity `text()^(-1)`

` = (0.248xx10^(-2) S cm^(-1) xx 1000 cm^3 L^(-1))/(0.02 mol L^(-1))`

` = 124 S cm^2 mol^(-1)`

Q 2987734687

The electrical resistance of a column of `0.05 mol L^(–1) NaOH` solution of diameter `1 cm` and length `50` cm is `5.55 × 10^3` ohm. Calculate its resistivity, conductivity and molar conductivity.

`A = pi r^2 = 3.14 xx (0.5)^2 cm^2 = 0.785 cm^2 = 0.785xx 10^(-4) m^2`

`R = ( rho l)/A ` or `rho = (RA)/l = (5.55xx10^3 Omega xx 0.785 cm^2)/(50 cm) = 87.135 Omega cm`

Conductivity = ` κ = 1/rho = 1/(87.135) S cm^(-1)`

` = 0.01148 S cm^(-1)`

Molar conductivity, ` Λ_m = (kappa xx1000)/c cm^3 L^(-1)`

` = (0.01148 S cm^(-1) xx 1000 cm^3 L^(-1))/(0.05 mol L^(-1))`

` = 229.6 S cm^2 mol^(-1)`

If we want to calculate the values of different quantities in terms of ‘m’ instead of ‘cm’,

`rho = (RA)/l = (5.55xx10^3 Omega xx 0.785 xx 10^(-4) m^2)/(0.5 m)`

` = 87.135xx10^(-2) Omega m`

`kappa = 1/rho = (100)/(87.135) Omega = 1.148 S m^(-1)` and `Λ_m = kappa/c = (1.148 S m^(-1))/(50 mol m^(-3))`

` = 229.6xx10^(-4) S m^2 mol^(-1)`

`=>` Both conductivity and molar conductivity changes with the concentration of the electrolyte.

`color{green}text(Variation of Conductivity) :` Conductivity always decreases with decrease in concentration both, for weak and strong electrolytes.

`color{green}("Explanation")` : The number of ions per unit volume that carry the current in a solution decreases on dilution. The conductivity of a solution at any given concentration is the conductance of one unit volume of solution kept between two platinum electrodes with unit area of cross section and at a distance of unit length. This is clear from the equation :

`color{red}(G = (k A)/l = k)` (both `A` and `l` are unity in their appropriate units in `m` or `cm`).

`color{green}(text(Variation of Molar Conductivity) ):` Molar conductivity of a solution at a given concentration is the conductance of the volume `V` of solution containing one mole of electrolyte kept between two electrodes with area of cross section `A` and distance of unit length. Therefore,

`color{red}(Λ_m = (k A)/l = k)` Since `l = 1` and `A = V` ( volume containing 1 mole of electrolyte) `color{red}(Λ_m = κ V)` .............(7).

Molar conductivity increases with decrease in concentration.

`color{green}("Explanation")` : The total volume, `V`, of solution containing one mole of electrolyte also increases. It has been found that decrease in `κ` on dilution of a solution is more than compensated by increase in its volume.

`Λ_m` can be defined as the conductance of the electrolytic solution kept between the electrodes of a conductivity cell at unit distance but having area of cross section large enough to accommodate sufficient volume of solution that contains one mole of the electrolyte.

`color{green}(text(Limiting Molar Conductivity)) :` When concentration approaches zero, the molar conductivity is known as limiting molar conductivity and is represented by the symbol `lamda_m^°`.

The variation in `Λ_m` with concentration is different (Fig. 3.6) for strong and weak electrolytes.

`color{green}text(Variation of Conductivity) :` Conductivity always decreases with decrease in concentration both, for weak and strong electrolytes.

`color{green}("Explanation")` : The number of ions per unit volume that carry the current in a solution decreases on dilution. The conductivity of a solution at any given concentration is the conductance of one unit volume of solution kept between two platinum electrodes with unit area of cross section and at a distance of unit length. This is clear from the equation :

`color{red}(G = (k A)/l = k)` (both `A` and `l` are unity in their appropriate units in `m` or `cm`).

`color{green}(text(Variation of Molar Conductivity) ):` Molar conductivity of a solution at a given concentration is the conductance of the volume `V` of solution containing one mole of electrolyte kept between two electrodes with area of cross section `A` and distance of unit length. Therefore,

`color{red}(Λ_m = (k A)/l = k)` Since `l = 1` and `A = V` ( volume containing 1 mole of electrolyte) `color{red}(Λ_m = κ V)` .............(7).

Molar conductivity increases with decrease in concentration.

`color{green}("Explanation")` : The total volume, `V`, of solution containing one mole of electrolyte also increases. It has been found that decrease in `κ` on dilution of a solution is more than compensated by increase in its volume.

`Λ_m` can be defined as the conductance of the electrolytic solution kept between the electrodes of a conductivity cell at unit distance but having area of cross section large enough to accommodate sufficient volume of solution that contains one mole of the electrolyte.

`color{green}(text(Limiting Molar Conductivity)) :` When concentration approaches zero, the molar conductivity is known as limiting molar conductivity and is represented by the symbol `lamda_m^°`.

The variation in `Λ_m` with concentration is different (Fig. 3.6) for strong and weak electrolytes.

For strong electrolytes, `Λ` increases slowly with dilution and can be represented by the equation

`Λ_m =Λ_m^° – A c^(½)`

It can be seen that if we plot `Λ_m` against `c^(1/2)`, we obtain a straight line with intercept equal to `Λ_m^°` and slope equal to `‘–A’`.

The value of the constant `‘A’` for a given solvent and temperature depends on the type of electrolyte i.e., the charges on the cation and anion produced on the dissociation of the electrolyte in the solution. Thus, `NaCl, CaCl_2, MgSO_4` are known as 1-1, 2-1 and 2-2 electrolytes respectively. All electrolytes of a particular type have the same value for ‘A’..

Kohlrausch examined `Λ_m^°` values for a number of strong electrolytes and observed certain regularities. He noted that the difference in `Λ_m^°` of the electrolytes `NaX` and `KX` for any `X` is nearly constant. For example at 298 K :

`color{red}(λ_(m(KCl))^0 - λ_(m (NaCl))^0 = λ_(m (KBr))^0 - λ_(m (NaBr))^0)`

`color{red}(= λ_(m(KI))^0 - λ_(m(NaI))^0 ≃ 23.4 S cm^2 mol^(-1))`

Similarly, it was found that `color{red}(λ_(m(NaBr))^0 -Λ_(m(NaCl))^0 = λ_(m(KBr))^0 ≃ 1.8 S cm^2 mol^(-1))`.

On the basis of the above observations he enunciated Kohlrausch law of independent migration of ions.

`color{green}text(Statement of Kohlrausch Law) :` Limiting molar conductivity of an electrolyte can be represented as the sum of the individual contributions of the anion and cation of the electrolyte.

Thus, if `λ_(Na^+)^0` and `λ_(Cl^-)^0` are limiting molar conductivity of the sodium and chloride ions respectively, then the limiting molar conductivity for sodium chloride is given by the equation :

`color{red}(λ_(m(NaCl))^0 = lamda_(Na^+)^0 + lamda_(Cl^-)^0)` ........(8)

In general, if an electrolyte on dissociation gives `v_+` cations and `v_-` anions then its limiting molar conductivity is given by :

`color{red}(λ_(m)^0 = v_+ lamda_(+)^0 + v_(-) lamda_(-)^0)` ..................(9).

Here `lamda_(+)^0` and `lamda_(-)^0` are the limiting molar conductivities of the cation and anion respectively. The values of `lamda^0` for some cations and anions at 298 K are given in Table

`Λ_m =Λ_m^° – A c^(½)`

It can be seen that if we plot `Λ_m` against `c^(1/2)`, we obtain a straight line with intercept equal to `Λ_m^°` and slope equal to `‘–A’`.

The value of the constant `‘A’` for a given solvent and temperature depends on the type of electrolyte i.e., the charges on the cation and anion produced on the dissociation of the electrolyte in the solution. Thus, `NaCl, CaCl_2, MgSO_4` are known as 1-1, 2-1 and 2-2 electrolytes respectively. All electrolytes of a particular type have the same value for ‘A’..

Kohlrausch examined `Λ_m^°` values for a number of strong electrolytes and observed certain regularities. He noted that the difference in `Λ_m^°` of the electrolytes `NaX` and `KX` for any `X` is nearly constant. For example at 298 K :

`color{red}(λ_(m(KCl))^0 - λ_(m (NaCl))^0 = λ_(m (KBr))^0 - λ_(m (NaBr))^0)`

`color{red}(= λ_(m(KI))^0 - λ_(m(NaI))^0 ≃ 23.4 S cm^2 mol^(-1))`

Similarly, it was found that `color{red}(λ_(m(NaBr))^0 -Λ_(m(NaCl))^0 = λ_(m(KBr))^0 ≃ 1.8 S cm^2 mol^(-1))`.

On the basis of the above observations he enunciated Kohlrausch law of independent migration of ions.

`color{green}text(Statement of Kohlrausch Law) :` Limiting molar conductivity of an electrolyte can be represented as the sum of the individual contributions of the anion and cation of the electrolyte.

Thus, if `λ_(Na^+)^0` and `λ_(Cl^-)^0` are limiting molar conductivity of the sodium and chloride ions respectively, then the limiting molar conductivity for sodium chloride is given by the equation :

`color{red}(λ_(m(NaCl))^0 = lamda_(Na^+)^0 + lamda_(Cl^-)^0)` ........(8)

In general, if an electrolyte on dissociation gives `v_+` cations and `v_-` anions then its limiting molar conductivity is given by :

`color{red}(λ_(m)^0 = v_+ lamda_(+)^0 + v_(-) lamda_(-)^0)` ..................(9).

Here `lamda_(+)^0` and `lamda_(-)^0` are the limiting molar conductivities of the cation and anion respectively. The values of `lamda^0` for some cations and anions at 298 K are given in Table

Q 2917034880

The molar conductivity of `KCl` solutions at different concentrations at `298 K` are given below:

Show that a plot between `Λ_m` and `c^(1/2)` is a straight line. Determine the values of `Λ_m^0` and `A` for` KCl`.

`c//mol L^(-1)` | `Λ_m//S cm^2 mol^(-1)` |
---|---|

`0.000198` | `148.61` |

`0.000309` | `148.29` |

`0.000521` | `147.81` |

`0.000989` | ` 147.09` |

Show that a plot between `Λ_m` and `c^(1/2)` is a straight line. Determine the values of `Λ_m^0` and `A` for` KCl`.

Taking the square root of concentration we obtain:

`c^(1/2)//(mol (L^(-1))^(1/2))` | `Λ_m//S cm^2 mol^(-1)` |
---|---|

`0.01407 ` | `148.61` |

`0.01758` | `148.29` |

`0.02283` | `147.81` |

`0.03145` | ` 147.09` |

A plot of `Λ_m`( y-axis) and `c^(1/2)` (x-axis) is shown in (Fig. ). It can be seen that it is nearly a straight line. From the intercept `(c^(1/2) = 0)`,

we find that `Λ_m^0 = 150.0 S cm^2 mol^(–1)` and `A = –` slope `= 87.46 S cm^2 mol^(–1)//(mol//L^(–1))^(1/2)`.

Q 2927134981

Calculate `Λ_m^0 ` for `CaCl_2` and `MgSO_4` from the data given in Table 3.4

We know from Kohlrausch law that

`Λ_(m (CaCl_2))^0 = lamda_(Ca^(2+))^0+2lamda_(Cl^(-))^0 = 119.0 S cm^2 mol^(-1) +2(76.3)S cm^2 mol^(-1) = 271.6S cm^2 mol^(-1)`.

`Λ_(m(MgSO_4))^0 = lamda_(Mg^(2+))^0 + lamda_(SO_4^(2-))^0 = 106.0 S cm^2 mol^(-1) +160.0 S cm^2 mol^(-1) = 266 S cm^2 mol^(-1)`.

Q 2917134989

`Λ_m^0` for `NaCl , HCl` and `NaAc` are `126.4 , 425 .9` and `91.0 S cm^2 mol^(-1)` respectively. Calculate `Λ^o` for `HAc`.

`Λ_(m (HAc))^0 = lamda_(H^+)^0 +lamda_(Ac^-)^0 = lamda_(H^+)^0 +lamda_(Cl^-)^0 +lamda_(Na^+)^0 - lamda_(Cl^-)^0 - lamda_(Na^+)^0`

`= Λ_(m (HCl))^0 +Λ_(m(NaAc))^0 - Λ_(m (NaCl))^0`

` = (425.9+91.0 - 126.4) S cm^2 mol^(-1)`

` = 390.5 S cm^2 mol^(-1)`

Weak electrolytes like acetic acid have lower degree of dissociation at higher concentrations and hence for such electrolytes, the change in `Λ_m` with dilution is due to increase in the degree of dissociation and consequently the number of ions in total volume of solution that contains 1 mol of electrolyte.

In such cases `λ_m` increases steeply (Fig) on dilution, especially near lower concentrations. Therefore, `Λ_m^°` cannot be obtained by extrapolation of `Λ_m` to zero concentration.

At infinite dilution (i.e., concentration c → zero) electrolyte dissociates completely (`α =1`), but at such low concentration the conductivity of the solution is so low that it cannot be measured accurately. Therefore, `λ_m^°` for weak electrolytes is obtained by using Kohlrausch law of independent migration of ions.

In such cases `λ_m` increases steeply (Fig) on dilution, especially near lower concentrations. Therefore, `Λ_m^°` cannot be obtained by extrapolation of `Λ_m` to zero concentration.

At infinite dilution (i.e., concentration c → zero) electrolyte dissociates completely (`α =1`), but at such low concentration the conductivity of the solution is so low that it cannot be measured accurately. Therefore, `λ_m^°` for weak electrolytes is obtained by using Kohlrausch law of independent migration of ions.

At any concentration `c`, if `α` is the degree of dissociation then it can be approximated to the ratio of molar conductivity `Λ_m` at the concentration `c` to limiting molar conductivity, `Λ_m^°`. Thus we have :

`color{red}(α = (Λ_m)/(Λ_m^0))` .........(10)

But we know that for a weak electrolyte like acetic acid,

`color{red}(K_a = (c α^2)/(1-α) = ( c Λ_m^2)/(Λ_m^(0^2)(1 - Λ_m/Λ_m^0)) = (c Λ_m^2)/(Λ_m^0(Λ_m^0-Λ_m)))` .......(3.27)

Using Kohlrausch law of independent migration of ions, it is possible to calculate `Λ_m^°` for any electrolyte from the `λ^o` of individual ions. Moreover, for weak electrolytes like acetic acid it is possible to determine the value of its dissociation constant once we know the `Λ_m^°` and `Λ_m` at a given concentration `c`.

`color{red}(α = (Λ_m)/(Λ_m^0))` .........(10)

But we know that for a weak electrolyte like acetic acid,

`color{red}(K_a = (c α^2)/(1-α) = ( c Λ_m^2)/(Λ_m^(0^2)(1 - Λ_m/Λ_m^0)) = (c Λ_m^2)/(Λ_m^0(Λ_m^0-Λ_m)))` .......(3.27)

Using Kohlrausch law of independent migration of ions, it is possible to calculate `Λ_m^°` for any electrolyte from the `λ^o` of individual ions. Moreover, for weak electrolytes like acetic acid it is possible to determine the value of its dissociation constant once we know the `Λ_m^°` and `Λ_m` at a given concentration `c`.

Q 2937345282

The conductivity of `0.001028 mol L^(-1)` acetic acid is `4.95xx10^(-5) S cm^(-1)` Calculate its dissociation constant if `Λ_m^0` for acetic acid is `390.5 S cm^2 mol^(-1)`.

`Λ_m = kappa/c = (4.95 xx 10^(-5) S cm^(-1))/(0.001028 mol L^(-1)) xx (1000 cm^3 )/L = 48.15 cm^2 mol^(-1)`

`alpha = Λ_m/(Λ_m^0) = (48.15 S cm^2 mol^(-1))/(390.5 S cm^2 mol^(-1)) = 0.1233`

`K = ( c alpha^2)/(1-alpha) = (0.001028 mol L^(-1) xx (0.1233)^2)/(1-0.1233) = 1.78xx10^(-5) mol L^(-1)`